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Sloan [31]
2 years ago
8

Carbon disulfide burns with oxygen to form carbon dioxide and sulfur dioxide in the following manner: CS2 + 3O2 → CO2 + 2SO2

Chemistry
1 answer:
Virty [35]2 years ago
4 0

Answer:

89.6 L.

Explanation:

  • For the balanced reaction:

<em>CS₂ + 3O₂ → CO₂ + 2SO₂.</em>

  • It is clear that <em>1.0 mole of CS₂</em> with 3.0 moles of O₂ to produce 1.0 mole of  CO₂ and <em>2.0 moles of SO₂.</em>

<em></em>

<u><em>Using cross multiplication:</em></u>

1.0 mole of CS₂ produces → 2.0 moles of SO₂.

2.0 mole of CS₂ produces → ??? moles of SO₂.

∴ The no. of moles of SO₂ produced = (2.0 mol)(2.0 mol)/(1.0 mol) = 4.0 mol.

  • It is known that 1.0 mole of any gas at STP occupies 22.4 L.

<em>∴ 4.0 moles of SO₂ occupy = (4.0)(22.4 L) = 89.6 L.</em>

<em></em>

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Zinc reacts with lead (II) nitrate to produce zinc nitrate and lead. This reactions is:
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Answer:

Displacement Reaction

Explanation:

Zinc replaces lead in Lead(ll) nitrate as zinc is more reactive than lead.

3 0
2 years ago
How many milliliters of a 0.211 M HI solution are needed to reduce 24.0 mL of a 0.354 M KMnO4 solution according to the followin
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Answer:

The answer to your question is 242 ml

Explanation:

Data

HI 0.211 M   Volume = x

KMnO₄ 0.354 M   Volume = 24 ml

Balanced Chemical reaction

     12HI + 2KMnO₄ + 2H₂SO₄ → 6I₂ + Mn₂SO₄ + K₂SO₄ + 8H₂O

Process

1.- Calculate the moles of KMnO₄  0.354 M in 24 ml

Molarity = moles / volume (L)

moles = Molarity x volume (L)

moles = 0.354 x 0.024

moles = 0.0085

2.- From the balanced chemical reaction we know that HI and KMnO₄ react in the proportion 12 to 2. Then,

              12 moles of HI --------------- 2 moles of KMnO₄

                x                     --------------- 0.0085 moles of KMnO₄

             x = (0.0085 x 12)/2

             x = 0.051 moles of HI

3.- Calculate the milliliters of HI 0.211 M

Molarity = moles/volume

Volume = moles/molarity

Volume = 0.051/0.211

Volume = 0.242 L or Volume = 242 ml

8 0
3 years ago
What is the volume of a solution that has a specific gravity of 1. 2 and a mass of 185g.
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8 0
3 years ago
Read 2 more answers
Sulfur burns in the air to form 33.6L of sulfur dioxide. (S = 32, O =16, 64g of sulfur dioxide has 22.4L, 32g of oxygen has 22.4
ivolga24 [154]

The mass of oxygen reacted/required in this reaction is obtained as 48g.

<h3>What is stoichiometry?</h3>

The term stoichiometry has to do with mass- volume or mass - mole relationship which ultimately depends on the balanced reaction equation.

Now, we have the reaction; S + O2 ------>SO2

If 1 mole of sulfur dioxide contains 22.4 L

x moles of sulfur dioxide contains 33.6L

x = 1.5 moles of sulfur dioxide.

Since the reaction is 1:1, the number if moles of oxygen required/reacted is 1.5 moles.

Mass of oxygen required/reacted = 1.5 moles * 32 g/mol = 48g

Learn more anout stoichiometry: brainly.com/question/9743981

8 0
2 years ago
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